Import Question JSON

Current Question (ID: 18224)

Question:

$\text{The number of electrons involved in the deposition of } 63.5 \text{ g of Cu from a solution of } \text{CuSO}_4 \text{ is:}$

Options:

1. $6.022 \times 10^{23}$
2. $3.011 \times 10^{23}$
3. $12.044 \times 10^{23}$
4. $6.022 \times 10^{22}$

Solution:

$\text{Step 1: Find the correct equation}$ $\text{Cu}^{+2} \rightarrow \text{Cu}$ $\text{Step 2: Find the number of electrons.}$ $\text{Cu}^{+2} + 2e^- \rightarrow \text{Cu}$ $\text{Step 3: According to Faraday's law, this equation requires 2F charge.}$ $1F \text{ charge} = \text{Charge carried by 1 mole of electrons}$ $2F \text{ charge} = \text{Charge carried by 2 moles of electrons}$ $2F \text{ charge} = 2 \times 6.023 \times 10^{23}$ $= 12.044 \times 10^{23}$

Import JSON File

Upload a JSON file containing LaTeX/MathJax formatted question, options, and solution.

Expected JSON Format:

{
  "question": "The mass of carbon present in 0.5 mole of $\\mathrm{K}_4[\\mathrm{Fe(CN)}_6]$ is:",
  "options": [
    {
      "id": 1,
      "text": "1.8 g"
    },
    {
      "id": 2,
      "text": "18 g"
    },
    {
      "id": 3,
      "text": "3.6 g"
    },
    {
      "id": 4,
      "text": "36 g"
    }
  ],
  "solution": "\\begin{align}\n&\\text{Hint: Mole concept}\\\\\n&1 \\text{ mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6] = 6 \\text{ moles of carbon atom}\\\\\n&0.5 \\text{ mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6] = 6 \\times 0.5 \\text{ mol} = 3 \\text{ mol}\\\\\n&1 \\text{ mol of carbon} = 12 \\text{ g}\\\\\n&3 \\text{ mol carbon} = 12 \\times 3 = 36 \\text{ g}\\\\\n&\\text{Hence, 36 g mass of carbon present in 0.5 mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6].\n\\end{align}",
  "correct_answer": 4
}